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- Four metals, A, B, C, and D, exhibit the following properties. (i) Only A and C react with 1.0 M hydrochloric acid to give H2(g). (ii) When C is added to solutions of the ions of the other metals, metallic B, D, and A are formed. (iii) Metal D reduces Bn+ to give metallic B and Dn+. Based on this information, arrange the four metals in order of increasing ability to act as reducing agents.arrow_forwardFor the reaction Cu2+(aq) + Zn(s) → Cu(s) + Zn2+ (aq), why can’t you generate electric current by placing a piece of copper metal and a piece of zinc metal in a solution containing CuCl2(aq) and ZnCl2(aq)?arrow_forwardIs the following statement true or false? Concentration cells work because standard reduction potentials are dependent on concentration. Explain.arrow_forward
- Calculate the equilibrium constant for the redox reactions that could occur in the following situations and use that value to explain whether or not any reaction will be observed. (a) A piece of iron is placed in a 1.0 M solution of NiCl2(aq). (b) A copper wire is placed in a 1.0 M solution of Pb(NO3)2(aq).arrow_forwardWhich of the following statement(s) is/are true? a. Copper metal can be oxidized by Ag+ (at standard conditions). b. In a galvanic cell the oxidizing agent in the cell reaction is present at the anode. c. In a cell using the half reactions Al3+ + 3e Al and Mg2+ + 2e Mg, aluminum functions as the anode. d. In a concentration cell electrons always flow from the compartment with the lower ion concentration to the compartment with the higher ion concentration. e. In a galvanic cell the negative ions in the salt bridge flow in the same direction as the electrons.arrow_forwardAs the voltaic cell shown here runs, the blue solution gradually gets lighter in color and the gray solution gets darker. (a) What species is oxidized and what is reduced? (b) Which electrode is the anode and which is the cathode? (C) Which metal electrode gains mass? (d) In which direction do electrons flow through the external circuit?arrow_forward
- Give the notation for a voltaic cell whose overall cell reaction is Mg(s)+2Ag+(aq)Mg2+(aq)+2Ag(s) What are the half-cell reactions? Label them as anode or cathode reactions. What is the standard cell potential of this cell?arrow_forwardFor a voltage-sensitive application, you are working on a battery that must have a working voltage of 0.85 V. The half-cells to be used have a standard cell potential of 0.97 V. What must be done to achieve the correct voltage? What information would you need to look up?arrow_forwardConsider a concentration cell that has both electrodes made of some metal M. Solution A in one compartment of the cell contains 1.0 M M2+. Solution B in the other cell compartment has a volume of 1.00 L. At the beginning of the experiment 0.0100 mole of M(NO3)2 and 0.0100 mole of Na2SO4 are dissolved in solution B (ignore volume changes), where the reaction M2+(aq)+SO42(aq)MSO4(s) occurs. For this reaction equilibrium is rapidly established, whereupon the cell potential is found to be 0.44 V at 25C. Assume that the process M2++2eM has a standard reduction potential of 0.31 V and that no other redox process occurs in the cell. Calculate the value of Ksp for MSO4(s) at 25C.arrow_forward
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